Episode Synopsis "Bronsted Acids and Bases: Types and Strength "

According to Bronsted-Lowry theory of acids and bases, - an acid is a proton, H3O+ or H+ donor - a base is a proton, H3O+ or H+ acceptor The strength of an acid or base is related to the extent of dissociation in solution: - a strong acid or base is fully dissociated - a weak acid or base is partially dissociated So therefore we will have 4 possible types of acids and bases: 1. Weak Acid 2. Strong Acid 3. Weak Base 4. Strong Base Also, each of these acids and bases will dissociate in solution to give different species. 1. Weak Acid Dissociation eg CH3COOH bronsted theory weak acid CH3COOH dissociation CH3COOH is a weak acid and dissociates partially in solution (as indicated with reversible arrow) to form H+ and CH3COO- ions. Since this is a reversible process, CH3COO- can accept H+ to form back CH3COOH. Therefore the nature of CH3COO- is basic and we call CH3COO- the conjugate base of CH3COOH. 2. Strong Acid Dissociation eg HCl bronsted theory strong acid HCl dissociation HCl is a strong acid and will dissociate fully (as indicated with full arrow) in solution to form H+ and Cl- ions. Since this is an irreversible process, Cl- has no tendency to accept H+ and form back HCl. Therefore the nature of Cl- is neutral. 3. Weak base dissociation eg NH3 bronsted theory weak base NH3 dissociation NH3 is a weak base and dissociates partially in solution (as indicated with reversible arrow) to form OH- and NH4+ ions. Since this is a reversible process, NH4+ can donate H+ to form back NH3. Therefore the nature of NH4+ is acidic and we call NH4+ the conjugate acid of NH3. 4. Strong base dissociation eg NaOH bronsted theory strong base NaOH dissociation NaOH is a strong base and will dissociate fully (as indicated with full arrow) in solution to form OH- and Na+ ions. Since this is an irreversible process, Na+ has no tendency to donate H+ and form back NaOH. Therefore the nature of Na+ is neutral. So in summary: - weak acid will dissociate to give conjugate base - weak base will dissociate to give conjugate acid - strong acid will dissociate to give a neutral ion - strong base will dissociate to give a neutral ion bronsted theory dissociation summary These concepts are fundamental and very important in Ionic Equilibria. Check out this video lesson to learn more about acids and bases and their dissociation in solution! Topic: Ionic Equilibria, Physical Chemistry, JC, H2, A Level Chemistry, Singapore You can also view this video lesson with screenshots and detailed explanation. Do check out the following for more video lessons: Physical Chemistry Videos  A Level Chemistry Videos  If you are looking for H2 Chemistry Tuition, do consider taking up my classes at Bishan or check out my online chemistry tuition lessons. 

Listen "Bronsted Acids and Bases: Types and Strength "

More episodes of the podcast A Level Chemistry Lessons

• How to deduce Nature of Salt in Salt Hydrolysis
• Bronsted Acids and Bases: Types and Strength 
• Balance Redox Reaction via Half Eqn Method 
• Compare Strength of 2 Acids with different pH 
• How to draw Amino Acids and Proteins
• Electrophilic Addition Mechanism for Alkenes
• How to compare Basicity of Amines, Phenylamines and Amides
• Saytzeff Rule, Zaitsev Rule: How to predict Major Product for Elimination Reaction
• Markovnikov Rule and Predicting Alkene Major Product